$Le-Chatelier$'s principle is not applicable to:

What is the effect of the reduction of the volume of the system for the equilibrium $2 C_{(s)} + O_{2(g)} \rightleftharpoons 2 CO_{(g)}$?

Explain the effect of a catalyst on chemical equilibrium with examples.

The equilibrium constant $K$ and reaction quotient $Q$ are in the ratio $K : Q = 0.33 : 1$. This means that:

When $I_2$ dissociates to its atomic form the following reaction occurs:
$I_{2(g)} \rightleftharpoons 2I_{(g)} ; \Delta_r H^o = +150 \ kJ \ mol^{-1}$
The forward reaction is favoured at:

The reaction,$N_{2(g)} + 3H_{2(g)} \rightleftharpoons 2NH_{3(g)}$ is exothermic and reversible. $A$ mixture of $N_{2(g)}$,$H_{2(g)}$,and $NH_{3(g)}$ is at equilibrium in a closed container. When a certain quantity of extra $H_{2(g)}$ is introduced into the container,while keeping the volume constant,then which statement among the following is true?